The number of mole of lithium, Li needed for the reaction is 3.2 moles (Option D)
<h3>Balanced equation </h3>
4Li + N₂(g) → 2Li₂N
From the balanced equation above,
2 moles of Li₂N were obtained from 4 moles of Li
<h3>How to determine the mole of lithium needed </h3>
From the balanced equation above,
2 moles of Li₂N were obtained from 4 moles of Li
Therefore,
1.6 moles of Li₂N will be obtained from = (1.6 × 4) / 2 = 3.2 moles of Li
Thus, 3.2 moles of Li are needed for the reaction
Learn more about stoichiometry:
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The energy transferred is 28.5 j
<em><u>calculation</u></em>
energy is calculate MCΔT formula where,
M(mass)= 6.30 grams
C(specific heat capacity)= 0.377 j/g
ΔT(change in temperature)= 32.0c- 20 c= 12 c
Energy is therefore= 6.30 g x 0.377 j/g /c x 12 c =<u>28.5 j</u>
1. To solve this question, you need to equalize the mass of solute for both solution. The calculation would be:
mass of solute= volume*concentration
mass1=mass2
volume1 * concentration1 = volume2 * concentration2
volume1 * 0.7%= 2L *(1000ml/L) * 0.2%
volume1 = 2000ml * (0.2%/0.7%)
volume1= 571.429 ml
2. Since you already have the volume of stock needed, you just need to subtract it from the total solution volume to count the number of solvents needed.
new solution volume= stock volume + diluting solvent volume
2L * 2000ml/L = 571.429ml + diluting solvent volume
diluting solvent volume= 2000ml- 571.429 ml= 1428.571ml
